The role of molecular oxygen (O₂) and UV light in the anion radical formation and stability of TCNQ and its fluorinated derivatives

Abstract

We report the electronic absorption spectroscopy of 7,7,8,8-tetracyanoquinodimethane (TCNQ) and its fluorinated derivatives (F2TCNQ and F4TCNQ), well-known electron-accepting molecules in common organic solvents (toluene, chlorobenzene, acetonitrile, and ethanol) under controlled exposure to air (O₂) and UV light. All compounds (FxTCNQ (x = 0, 2, 4)) were stable in a neutral state (FxTCNQ⁰) in toluene and chlorobenzene, even under both O₂ and UV light. On the other hand, in EtOH, the formation of FxTCNQ^·− was monitored upon controlled exposure to O₂ or UV light. Especially in air-equilibrated ethanol upon the UV-illumination, efficient α,α-dicyano-p-toluoylcyanide anion (DCTC⁻) and its fluorinated derivatives were generated evinced by the absorption peak near 480 nm, whereas the reaction was shut off by removing O₂ or blocking UV light, thereby keeping FxTCNQ^·− stable. However, even in deaerated ethanol, upon the UV-illumination, the anion formation of TCNQ and its fluorinated derivatives (FxTCNQ^·−, x = 0, 2, 4) was inevitable, showing the stability of FxTCNQ⁰ depends on the choice of solvent.

Introduction

Organic semiconducting molecules have received attention for their applications in biosensors, nonlinear optics, transistors, optoelectronics due to their nontoxicity, bandgap tunability, facile fabrication, and flexibility (Kim et al. 2022; Cha et al. 2020; Bronstein et al. 2020; Yuan et al. 2019; Sun et al. 2019; Oh et al. 2019; Hiramoto et al. 2019; Yu et al. 2018; Wang et al. 2018; Nayak et al. 2016; Feier et al. 2016; Mishra and Bäuerle 2012; Hains et al. 2010; Coropceanu et al. 2007; Suchanski and Duyne 1976; Yanti et al. 2021). Despite an intrinsically large exciton binding energy (E_B >  ~ 100 meV–1 eV) in organic semiconductors, organic charge transfer (CT) complexes have shown strikingly high conductivity (σ > 10² S cm^–1), comparable to metals (Saito and Yoshida 2007). These molecular electronics have motivated the synthesis of new functional molecules, and their optical/electrical/photophysical properties have been examined.

7,7,8,8-tetracyanoquinodimethane (TCNQ) in Fig. 1 is a well-known electron-acceptor molecule and has been utilized in various molecular electronics with its LUMO energy level at − 4.23 eV (Kanai et al. 2009) that matches well with diverse electron donor molecules to produce functional CT complexes (Zhang et al. 2018). TCNQ undergoes one or two electron reduction reactions to form stable anion by-products, TCNQ^·− and TCNQ²⁻ (Vishwanath et al. 2019). Previously, the spontaneous formation of α,α-dicyano-p-toluoylcyanide anion (DCTC⁻) has been observed in TCNQ solution. Several potential mechanisms have been proposed (Ning et al. 2019; Hertler et al. 1962; Mizoguchi et al. 1978; Kryszewski et al. 1981; Grossel et al. 2000; Le et al. 2011), one of which includes the reaction of reduced TCNQ²⁻ with dissolved O₂(g) to produce DCTC⁻ in ambient solution (Ning et al. 2019). On the other hand, several conflicting mechanisms of the formation of DCTC⁻, involving neutral TCNQ or TCNQ^·− also have been reported as well (Hertler et al. 1962; Mizoguchi et al. 1978; Kryszewski et al. 1981; Grossel et al. 2000).

Fig. 1

Molecular structures of TCNQ, F2TCNQ, and F4TCNQ

For further energy level engineering, several fluorinated derivatives, tetrafluorinated/difluorinated TCNQ (F4TCNQ and F2TCNQ), were developed and successfully have shown the tunability of the first reduction potential with respect to TCNQ: E_1/2(TCNQ^·−/TCNQ) = − 54 mV; E_1/2(F2TCNQ^·−/F2TCNQ) =  + 165 mV; E_1/2(F4TCNQ^·−/F4TCNQ) =  + 365 mV versus Ag/Ag⁺ in CH₃CN (Le et al. 2011; Miyasaka et al. 2010). Furthermore, these fluorinated TCNQ derivatives have been shown to form radical anions and dianions in polar solvents such as acetonitrile and ethanol (Ma et al. 2014; Vo et al. 2018; Chae et al. 2014), while external conditions such as O₂ or UV light for anion species formation have not been well characterized. Therefore, to utilize the electron-accepting property of TCNQ and its fluorinated derivatives in many devices, it is crucial to understand the conditions to keep TCNQ derivatives neutral (TCNQ⁰) and to prevent from producing by-products such as anions or DCTC⁻. In this regard, the role of O₂ and UV light on the spectroscopic properties of TCNQ derivatives is worth investigating. Here, we report the electronic absorption spectroscopy of 7,7,8,8-tetracyanoquinodimethane (TCNQ) and its fluorinated derivatives (F2TCNQ and F4TCNQ) in various common organic solvents (toluene-Tol, chlorobenzene-CB, acetonitrile-ACN, and ethanol-EtOH) either as air-equilibrated or as N₂-purged with controlled UV-illumination. TCNQ showed the production of DCTC⁻ upon the reaction of TCNQ^·− with O₂ in EtOH under UV-illumination, whereas in N₂-purged EtOH, no or minimal DCTC⁻ was observed. On the other hand, stable neutral form TCNQ⁰ was confirmed in Tol, CB, or ACN. Similarly, F2TCNQ and F4TCNQ in air-equilibrated EtOH exhibited the effective production of fluorinated DCTC⁻ derivatives with an absorption peak near 480 nm under UV, which was suppressed by removing O₂ or blocking UV light.

Experimental section

Materials

7,7,8,8-tetracyanoquinodimethane (TCNQ), 2,5-Difluoro-7,7,8,8-tetracyanoquinodimethane (F2TCNQ), and tetrafluorotetracyanoquinodimethane (F4TCNQ, purified from sublimation) were purchased from Tokyo Chemical Industry (TCI) and used without further purification. Ethanol (HPLC/spectrophotometric grade, Sigma-Aldrich), acetonitrile (HPLC/spectrophotometric grade, J. T. Baker), toluene (HPLC grade, Wako Chemicals), and chlorobenzene (HPLC grade, Sigma-Aldrich) were used as received.

Instrumentation

Electronic absorption spectra were acquired using a Hitachi U-3900 UV/visible/NIR spectrophotometry system in a quartz optical cell. Baseline corrections for the transmittance of an optical cell with solvent were made prior to each measurement. In addition, the evolution of an absorption spectrum upon the UV-illumination (365 nm, 4 W, CW UV lamp) was monitored either with molecular oxygen in an air-equilibrated solution or without molecular oxygen in an N₂ (99.999% purity)-purged solution to examine the absorption behavior of TCNQ derivatives, dependent on the presence of O₂.

Results and discussion

To fabricate OPV devices or to prepare solution samples for photocatalyst characterization, electrical or photophysical studies involving TCNQ, solution processes are commonly used. In this regard, electronic absorption spectra of TCNQ were explored in various common organic solvents: toluene (Tol), chlorobenzene (CB), acetonitrile (ACN), and ethanol (EtOH). Additional file 1: Figure S1 displays the electronic absorption spectra of TCNQ in air-equilibrated solvents, and the spectroscopic results are tabulated in Table 1. In all solvents, the absorption spectra of TCNQ revealed the characteristic S₀ → S₁ transition in the range of 394–403 nm, consistent with the previous literature results (Suchanski and Duyne 1976). However, in Additional file 1: Figure S1d (black line), TCNQ in EtOH displays additional dual peaks in 700–900 nm, which are typical peaks for TCNQ anion radical (TCNQ^·−) (Melby et al. 1962).

Table 1 Electronic absorption spectroscopic data

The spectroscopic behavior of TCNQ was further tracked upon UV light illumination every 3-min to examine its photostability for a total of 15 min, as shown in Fig. 2a, Additional file 1: Figures S1 and S3. The spectroscopic results of TCNQ, either in air-equilibrated Tol, CB, or ACN, showed a virtually consistent absorption spectrum. In contrast, TCNQ in air-equilibrated EtOH (EtOH-air) exhibited a substantial drop of the intensity for the absorption band at 396 nm even in 3 min in Fig. 2a. With the decrease of 396 nm band, multiple absorption bands at 421, 743, and 841 nm, corresponding to TCNQ^·− increased, and a new band at 474 nm emerged. At 6 min (green in Fig. 2a), even the absorption bands of TCNQ^·− at 421, 743, and 841 nm began to decrease, and the 474 nm band continuously gained its intensity up to 15 min (magenta line in Fig. 2a), when the original absorption peak at 396 nm was wholly disappeared. The spectral change for TCNQ in EtOH-air in Fig. 2a suggests that TCNQ reacted to generate TCNQ^·−, in contrast to stable TCNQ⁰ in Tol, CB, or ACN. Furthermore, the spectral evolution upon the UV-illumination from 3 to 15 m, featuring the decrease of 743 and 841 nm band, implies that TCNQ^·− was reacted to produce the species that shows an absorption peak at 474 nm. The new species that shows the absorption band at 474 nm has been ascribed to α,α-dicyano-p-toluoylcyanide anion (DCTC⁻, Additional file 1: Figure S2) previously (Suchanski and Duyne 1976; Hertler et al. 1962; Mizoguchi et al. 1978; Kryszewski et al. 1981; Grossel et al. 2000; Xiulan et al. 2012), and the details of DCTC⁻ generation are discussed below. No sign of TCNQ²⁻ with a peak at ~ 330 nm was observed during this spectroscopic evolution, contrasting to the previous studies in ACN (Suchanski and Duyne 1976; Chae et al. 2014).

Fig. 2

a–c Comparative electronic absorption spectral evolution of TCNQ in a air-equilibrated, b degassed EtOH as a function of UV-illumination time, and in c air-equilibrated EtOH as a function of time without UV-illumination

Due to the potential role of molecular oxygen (O₂) in air-equilibrated EtOH in DCTC⁻ generation, the spectroscopic behavior of TCNQ was further examined in degassed EtOH (EtOH-N₂) by pre-purging EtOH solvent and purging TCNQ solution in EtOH with high purity (99.999%) N₂ gas. Figure 2b displays the spectral evolution upon the same UV-illumination. Like the absorption spectrum of TCNQ in EtOH-air at 0 m in Fig. 2a (black line), TCNQ in EtOH-N₂ also exhibited the characteristic 396 nm band for TCNQ⁰ in addition to 743 and 841 nm bands corresponding to TCNQ^·− in Fig. 2b (black line). At 3 m (red line), TCNQ^·− peaks increased with the decrease of TCNQ peak, and the additional band at 421 nm is also the spectroscopic fingerprint of TCNQ^·−, which was buried with TCNQ⁰ band at 0 m due to the spectral proximity. From 6 min (green line), the spectral change in EtOH-N₂ contrasts with that in EtOH-air, lacking the growth of the DCTC⁻ absorption band at 474 nm. Also, the absorption peak intensity of TCNQ^·− peaks in EtOH-N₂ was kept constant, suggesting stable TCNQ^·− and no further reactions consuming TCNQ^·− occurred. The formation of DCTC⁻ in EtOH-N₂ could be blocked because of the absence of TCNQ^·− even without O₂. Additional file 1: Figure S4 presents the absorption spectra of TCNQ as a function of time passed since blocking UV light in the middle of UV-illumination (exposed to UV light for 9 min), clearly showing the presence of TCNQ^·−. Over the 10 min since blocking UV light, no DCTC⁻ generation was noticed, highlighting the role of both O₂ and TCNQ^·−.

Since the initial report of TCNQ, several DCTC⁻ generation mechanisms from TCNQ have been proposed, whether the reaction starts either from TCNQ⁰, TCNQ^·−, or TCNQ²⁻ (Hertler et al. 1962; Mizoguchi et al. 1978; Kryszewski et al. 1981; Grossel et al. 2000; Xiulan et al. 2012). To identify the origin of DCTC⁻ formation, we plotted the absorbance (Abs₄₇₄) of DCTC⁻ product, monitored at 474 nm against the absorbance (Abs₈₄₁) of TCNQ^·− at 841 nm using the data in Fig. 2a. If DCTC⁻ is produced from TCNQ^·−, as the stoichiometry of TCNQ^·− and DCTC⁻ is 1:1 based upon the potential mechanism shown in Additional file 1: Figure S2, the concentration of the produced DCTC⁻ ([DCTC⁻]_p,t) at a given t should be equivalent to that of the consumed TCNQ^·− ([TCNQ^·−]_c,t) at the same t.

$$\left[ {{\text{DCTC}}^{ - } } \right]_{{{\text{p}},{\text{t}}}} = \, \left[ {{\text{TCNQ}}^{ \cdot - } } \right]_{{{\text{c}},{\text{t}}}}$$

(1)

From the Beer’s law:

$$\left[ {{\text{DCTC}}^{ - } } \right]_{{{\text{p}},{\text{t}}}} = {\text{Abs}}_{{{474}}} /\varepsilon_{{{474}}} \left( {{\text{DCTC}}^{ - } } \right)$$

(2)

$$\left[ {{\text{TCNQ}}^{ \cdot - } } \right]_{{{\text{c}},{\text{t}}}} = \, - {\text{Abs}}_{{{841}}} /\varepsilon_{{{841}}} \left( {{\text{TCNQ}}^{ \cdot - } } \right)$$

(3)

where ε_x(A) is the molar absorption coefficient at x nm for A species. Therefore, from the equivalence in Eq. (1) as well as Eqs. (2) and (3), the Abs₄₇₄ should be linearly proportional to Abs₈₄₁ as in Eq. (4), and the proportionality constant would be the ratio of ε₄₇₄(DCTC⁻) to ε₈₄₁(TCNQ^·−):

$${\text{Abs}}_{{{474}}} = \, - \left[ {\varepsilon_{{{474}}} \left( {{\text{DCTC}}^{ - } } \right)/\varepsilon_{{{841}}} \left( {{\text{TCNQ}}^{ \cdot - } } \right)} \right]{\text{Abs}}_{{{841}}}$$

(4)

Figure 3a displays the Abs₄₇₄(DCTC⁻) against Abs₈₄₁(TCNQ^·−), and the linear fit determined the proportionality constant to be −0.814 (± 0.03). From the literature, ε₄₇₄(DCTC⁻) and ε₈₄₁(TCNQ^·−) have been reported in various solvents. Using ε₄₇₄(DCTC⁻) = 38,800 cm⁻¹ M⁻¹ and ε₈₄₁(TCNQ^·−) = 43,500 cm⁻¹ M⁻¹ in acetone (Hertler et al. 1962; Grossel et al. 2000; Melby et al. 1962), ε₄₇₄(DCTC⁻)/ε₈₄₁(TCNQ^·−) can be calculated to be 0.892, which matches reasonably well despite the solvent difference. In addition, Abs₈₄₁(TCNQ^·−) is plotted against the UV-illumination time in Fig. 3b, showing the pseudo-first-order reaction for TCNQ^·− behavior is observed, again supporting that the reaction of TCNQ^·− is not mediated by the self-collisions, consistent with the proposed mechanism by Hipps et al. (Qi et al. 2012) and the resulting fit determined the rate constant to be 0.13 m⁻¹.

Fig. 3

a Plot of Abs₄₇₄(DCTC⁻) against Abs₈₄₁(TCNQ^·−) and its linear fit (blue line). b Plot of the natural log (ln(Abs₈₄₁(TCNQ^·−)) for Abs₈₄₁(TCNQ^·−) as a function of UV-illumination time and its linear fit (blue line)

Structurally related fluorinated TCNQ molecules (F2TCNQ and F4TCNQ: FxTCNQ, x = 2 and 4) have been widely utilized as comparative and tunable functional molecules to TCNQ, as their spectroscopic signatures are similar in spite of the modified reduction energy levels. The absorption spectra of FxTCNQ, either EtOH-air or EtOH-N₂, in Fig. 4a, b, d, e showed substantial change over time, like TCNQ in EtOH. On the other hand, as presented in Additional file 1: Figure S5a, b, d, e, no appreciable spectral change was probed in Tol or CB even under UV-illumination, while in ACN, F4TCNQ showed a noticeable decrease in 387 nm band, contrasting to F2TCNQ that displayed no spectral change (Figure S5c, f). This is likely due to the higher electron affinity of F4TCNQ, resulting in the reduction of F4TCNQ. On the other hand, in EtOH-air, both F2TCNQ and F4TCNQ in Fig. 4a, b, d, e displayed a dramatic change as in TCNQ. As the formation of an oxidized product, DCTC⁻ from TCNQ^·− was evident from a new absorption band at ~ 480 nm in Fig. 2a, F2TCNQ and F4TCNQ in EtOH-air similarly show the rise of ~ 480 nm band under UV light. Congruent to TCNQ, in EtOH-N₂, the effective growth of the 480 nm band was not observed, again suggesting that fluorinated DCTC⁻ derivatives were not produced without O₂. Additionally, even in EtOH-air, without UV light, FxTCNQ^·− (x = 0, 2, 4) was not effectively generated in Fig. 4c, f, evincing the stable neutral TCNQ⁰ and F2TCNQ⁰, contrary to unstable F4TCNQ that underwent F4TCNQ²⁻ formation (Melby et al. 1962).

Fig. 4

a–f Comparative electronic absorption spectral evolution of a–c F2TCNQ and d–f F4TCNQ in a, c air-equilibrated, b, d degassed EtOH as a function of UV-illumination time, and those in c, f air-equilibrated EtOH as a function of time without UV-illumination

Conclusions

In summary, the electronic absorption spectroscopy of FxTCNQ (x = 0, 2, 4) probed the stability of FxTCNQ (x = 0, 2, 4) in common organic solvents upon controlled exposure to O₂ or UV light. In general, all FxTCNQ compounds were stable in Tol and CB even under both O₂ and UV light, whereas in EtOH, the FxTCNQ^·− formation was monitored. Furthermore, in air-equilibrated EtOH upon UV-illumination, efficient α,α-dicyano-p-toluoylcyanide anion (DCTC⁻) and its fluorinated derivatives were generated, whereas the reaction was shut off by removing O₂ or blocking UV light. With the significance of TCNQ and its derivatives (F2TCNQ and F4TCNQ) not only in molecular electronics but also in electrochemistry, this work will provide an understanding of the impact of external stimuli such as O₂ and UV light on TCNQ compounds.